Kinetics
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
5. In the following reaction, the rate of formation of NH3 is 0.15 mol/L•min. What is the rate of reaction?
N2 + 3H2
2NH3
a. 0.15 mol/L•min
b. 0.075 mol/L•min
c. -0.075 mol/L•min
d. 0.20 mol/L•min
e. 0.30 mol/L•min
____
6. In the following reaction,
____
____
= -0.89 mol/L•s. What is the value of the rate of the reaction at this time?
A + 3B AB3
a. 0.30 mol/L•s
b. 0.89 mol/L•s
c. -0.30 mol/L•s
d. 2.67 mol/L•s
e. 0.22 mol/L•s
7. Consider the exothermic combustion of coal. Which of the following could increase the rate of reaction?
a. using smaller pieces of coal
b. increasing the concentration of oxygen
c. lowering the temperature
d. both (a) and (b) are correct
e. choices (a), (b) and (c) are all correct
8. Suppose a reaction A + B C occurs at some initial rate at 25°C. Which response includes all of the changes
below that could increase the rate of this reaction?
I.
II.
III.
lowering the temperature
adding a catalyst
increasing the initial concentration of B
a. I
b. II
c. III
d. I and II
e. II and III
____ 9. Which response below is not an example of how the nature of reactants affects the rate of reaction?
a. Graphite burns faster than diamond under equal conditions.
b. Coal dust burns faster than large chunks of coal.
c. Magnesium reacts faster in higher concentrations of HCl(aq).
d. Calcium reacts faster in water than magnesium.
e. White phosphorus reacts explosively on contact with air; red phosphorus does not.
____ 10. Which of the following reactions would be expected to be the slowest?
a. Ag+(aq) + Cl-(aq) AgCl(s)
b. H+(aq) + OH-(aq) H2O( )
c. CH4(g) + 2O2(g)
CO2(g) + 2H2O(g)
____ 11.
____ 12.
____ 13.
____ 14.
____ 15.
____ 16.
____ 17.
d. Pb2+(aq) + CrO42-(aq) PbCrO4(s)
e. H+(aq) + CN-(aq) HCN(aq)
Which is not an example of the effect of subdivision of the reactant on the rate of chemical reaction?
a. Violent explosions that occur in grain elevators.
b. A container of flammable liquid will burn on the surface but allowed to vaporize will burn
explosively.
c. A chunk of iron takes months to rust completely while iron wool will rust in days.
d. Some metals may be fused (welded) with minimal loss while their powders will burn in a
flame.
e. The Grand Canyon was created by dissolution by water over millions of years.
For a given reaction, the rate-law expression is ____.
a. a constant of proportionality between reaction rate and the concentrations of reactants
b. the sum of the powers to which reactant concentrations appear
c. an equation in which reaction rate is equal to a mathematical expression involving, or
related to, concentrations of reactants involved in the rate-determining step
d. an equation that gives the additional energy that reactants must obtain in order to react
e. 55 miles per hour
Which of the following statements about reaction orders in the rate law expression is incorrect?
a. Their values may equal the stoichiometric coefficients in the balanced equation.
b. Their values may or may not equal the stoichiometric coefficients in the balanced
equation.
c. Their values must be experimentally determined.
d. Their values get larger as the temperature is increased.
e. An order equal to zero means there is no concentration dependence with rate.
The gas phase reaction A + B
C has a reaction rate which is experimentally observed to follow the
relationship rate = k[A]2[B]. The overall order of the reaction
a. is first.
b. is second.
c. is third.
d. is zero.
e. is one-half.
The gas phase reaction A + B + C
D has a reaction rate which is experimentally observed to follow the
relationship rate = k[A]2[C]. The reaction is ____ order in A, ____ order in B, and ____ order in C.
a. first, second, third
b. first, second, zero
c. second, zero, first
d. second, first, zero
e. second, zero, zero
The gas phase reaction A + B
C has a reaction rate which is experimentally observed to follow the
relationship rate = k[A]2[B]. Which one of the following would affect the value of the specific rate constant,
k?
a. decreasing the temperature
b. changing the concentration of A
c. changing the concentration of B
d. changing the concentration of C
e. letting the reaction go on for a long time
A hypothetical reaction X + 2Y
Products is found to be first order in X and second order in Y. What are
the units of k, the specific rate constant, if reaction rate is expressed in units of moles per liter per second?
a. M•s-1
____ 18.
____ 19.
____ 20.
____ 21.
____ 22.
____ 23.
____ 24.
b. M-2•s-1
c. M-3•s
d. M2•s-1
e. M-1•s
Which of the following statements regarding the rate constant in the rate law expression is incorrect?
a. Its value increases with temperature.
b. Its value is independent of initial concentration at a given temperature.
c. Its units depend on the overall order of reaction.
d. Its value is experimentally determined.
e. The larger its value, the slower the reaction rate.
A reaction A + 2B C is found to be first order in A and first order in B. What are the units of the rate
constant, k, if the rate is expressed in units of moles per liter per minute?
a. M-1•min-1
b. M
c. M•min-1
d. min-1
e. M2•min-1
Consider the following rate law expression: rate = k[A]2[B]. Which of the following is not true about the
reaction having this expression?
a. The reaction is first order in B.
b. The reaction is overall third order.
c. The reaction is second order in A.
d. A and B must both be reactants.
e. Doubling the concentration of A doubles the rate.
Consider the following rate law expression: rate = k[A][B]2. If the concentration of A is tripled and the
concentration of B is reduced by half, what is the resulting change in the reaction rate?
a. The rate is increased by 3/2.
b. The rate is reduced by 3/4.
c. The rate stays the same.
d. The rate is doubled.
e. The rate is reduced by 1/2.
The gas phase reaction A + B
C has a reaction rate which is experimentally observed to follow the
relationship rate = k[A]2[B]. If the concentration of A is tripled and the concentration of B is doubled, the
reaction rate would be increased by a factor of ____.
a. 6
b. 9
c. 12
d. 18
e. 36
The gas-phase reaction
2NO + 2H2
N2 + 2H2O
has the following rate law expression, rate = k[NO]2[H2]. If the [NO] is halved and the [H2] is tripled, what
change in rate is expected?
a. decrease by 3/4
b. increase by 3/4
c. increase by 3/2
d. decrease by 3/2
e. stays same
The gas-phase reaction
2NO + 2H2
N2 + 2H2O
has the following rate law expression, rate = 0.14 L2/mol2•s[NO]2[H2]. If the [NO] is 0.95 M and the [H2] is
0.45 M, what rate is expected?
a. 0.060 mol/L•s
b. 0.43 mol/L•s
c. 0.027 mol/L•s
d. 1.54 mol/L•s
e. 0.057 mol/L•s
____ 25. A reaction is second order in X and zero order in Y. Doubling the initial concentration of X and halving the
initial concentration of Y at constant temperature causes the initial rate to
a. increase by a factor of 4.
b. decrease by a factor of 2.
c. remain unchanged.
d. increase by a factor of 2.
e. be undeterminable without the balanced equation.
____ 26. Consider the following rate data for the reaction below at a particular temperature.
2A + 3B
Experiment
1
2
3
Initial [A]
0.10 M
0.10 M
0.20 M
Initial [B]
0.30 M
0.60 M
0.90 M
Products
Initial Rate of Loss of A
7.20  10-5 M•s-1
1.44  10-4 M•s-1
8.64  10-4 M•s-1
The reaction is ____ order in A and ____ order in B.
a. first, first
b. second, first
c. first, second
d. second, second
e. third, first
____ 27. Given the following data for the NH4+ + NO2N2 + 2H2O reaction
Trial
1
2
3
[NH4+]
0.010 M
0.015
0.010
[NO2-]
0.020 M
0.020
0.010
Rate
0.020 M/s
0.030
0.005
The rate law for the reaction is
a. rate = k[NH4+][NO2-]
b. rate = k[NH4+]2[NO2-]
c. rate = k[NH4+][NO2-]2
d. rate = k[NH4+]2[NO2-]2
e. None of the above
____ 28. Determine the rate-law expression for the reaction below.
2A + B2 + C A2B + BC
Trial
1
2
Initial [A]
0.20 M
0.40 M
Initial [B2]
0.20 M
0.30 M
Initial [C]
0.20 M
0.20 M
Initial Rate of Formation of BC
2.4  10-6 M•min-1
9.6  10-6 M•min-1
3
4
0.20 M
0.20 M
0.30 M
0.40 M
2.4  10-6 M•min-1
4.8  10-6 M•min-1
0.20 M
0.40 M
a. rate = k[A]2[B2][C]
b. rate = k[B2]2[C]2
c. rate = k[A][C]2
d. rate = k[A]2[C]
e. rate = k[A][B2][C]
____ 29. Rate data have been determined at a particular temperature for the overall reaction 2NO + 2H2
in which all reactants and products are gases.
Trial Run
1
2
3
Initial [NO]
0.10 M
0.10 M
0.20 M
Initial [H2]
0.20 M
0.30 M
0.20 M
N2 + 2H2O
Initial Rate (M•s-1)
0.0150
0.0225
0.0600
The rate-law expression is ____.
a. rate = k[NO]2[H2]2
b. rate = k[NO][H2]2
c. rate = k[NO]2[H2]
d. rate = k[NO][H2]
e. None of the preceding answers is correct.
____ 30. A troublesome reaction that is responsible in part for acid rain is
SO3 + H2O H2SO4
Rate data have been determined at a particular temperature for the reaction in which all reactants and products
are gases.
Trial Run
1
2
3
4
Initial [SO3]
0.35 M
0.70 M
0.35 M
0.70 M
Initial [H2O]
0.35 M
0.35 M
0.70 M
0.70 M
Initial Rate (M•s-1)
0.150
0.600
0.300
1.20
The rate-law expression is ____.
a. rate = k[SO3]2[H2O]2
b. rate = k[SO3]2[H2O]
c. rate = k[SO3][H2O]2
d. rate = k[SO3]2
e. rate = k[SO3][H2O]
____ 31. NO reacts with chlorine in a gas phase reaction to form nitrosyl chloride, NOCl. From the following
experimental data, determine the form of the equation that describes the relationship of reaction rate to initial
concentrations of reactants.
2NO + Cl2
Run
1
2
3
Initial [NO]
0.50 M
1.00 M
1.00 M
Initial [Cl2]
0.50 M
1.00 M
0.50 M
2NOCl
Initial Rate of
Formation of NOCl
1.14 M/hr
9.12 M/hr
4.56 M/hr
a. rate = k[NO]
b. rate = k[NO][Cl2]
c. rate = k[NO]2
d. rate = k[NO]2[Cl2]
e. rate = k[NO]2[Cl2]2
____ 32. The following data were collected for the following reaction at a particular temperature. What is the rate-law
expression for this reaction? rate = ____.
A+B
Experiment
1
2
3
Initial [A]
0.10 M
0.20 M
0.10 M
Initial [B]
0.10 M
0.20 M
0.20 M
C
Initial Rate of Formation of C
4.0  10–4 M/min
3.2  10–3 M/min
1.6  10–3 M/min
a. k[A]
b. k[A]2
c. k[A][B]
d. k[B]
e. k[A][B]2
____ 33. The following data were collected for the following reaction at a particular temperature. What is the rate-law
expression for this reaction? rate = ____.
Experiment
1
2
3
Initial [NH3]
1.10 M
2.20 M
1.10 M
NH3 + O2
N2O + H2O
Initial [O2]
1.10 M
2.20 M
2.20 M
Initial Rate
5.5  10–3 M/s
4.4  10–2 M/s
2.2  10–2 M/s
a. k[NH3]
b. k[NH3]2
c. k[NH3][ O2]
d. k[O2]
e. k[NH3][ O2]2
____ 34. Determine the rate-law expression for the reaction below at the temperature at which the tabulated initial rate
data were obtained. rate = ____
Experiment
1
2
3
4
a.
b.
c.
d.
e.
k[A][B]
k[A]2[C]
k[C]2
k[B]2[C]
none of these
Initial [A]
0.10 M
0.40 M
0.20 M
0.20 M
A + 2B + 3C Products
Initial [B]
Initial [C]
Initial Rate of Loss of A
0.20 M
0.10 M
4.0  10–2 M•min–1
0.20 M
0.10 M
4.0  10–2 M•min–1
0.20 M
0.25 M
1.0  10–1 M•min–1
0.40 M
0.10 M
1.6  10–1 M•min–1
____ 35. Evaluate the specific rate constant for this reaction at 800°C. The rate-law expression is rate = k[NO]2[H2].
(Choose the closest answer.)
2NO(g) + 2H2(g)
(g) + 2H2O(g)
Experiment Initial [NO]
Initial [H2]
Initial Rate of Reaction (M•s-1)
1
0.0010 M
0.0060 M
7.9  10-7
2
0.0040 M
0.0060 M
1.3  10-5
3
0.0040 M
0.0030 M
6.4  10-6
a. 22 M-2•s-1
b. 4.6 M-2•s-1
c. 1.3  102 M-2•s-1
d. 0.82 M-2•s-1
e. 0.024 M-2•s-1
____ 36. Evaluate the specific rate constant for the reaction at the temperature for which the data were obtained. The
rate-law expression is rate = k[A][B]2.
Experiment
1
2
3
Initial [A]
0.10 M
0.20 M
0.10 M
A+B
Initial [B]
0.10 M
0.20 M
0.20 M
C
Initial Rate of Formation of C
4.0  10–4 M/min
3.2  10–3 M/min
1.6  10–3 M/min
a. 1.2  10-2 M-2•min-1
b. 3.6  10-2 M-2•min-1
c. 4.0  10-1 M-2•min-1
d. 6.2  10-1 M-2•min-1
e. 7.0  10-3 M-2•min-1
____ 37. Evaluate the specific rate constant at the temperature at which the data were collected. The rate-law
expression is rate = k[NO]2[H2].
Experiment
1
2
3
H2(g) + NO(g)
N2O(g) + H2O(g)
Initial [NO] (M)
Initial [H2] (M)
Initial Rate (M•s–1)
0.30
0.35
2.835  10–3
0.60
0.35
1.134  10–2
0.60
0.70
2.268  10–2
a. 9.4  10-3 M-2•s-1
b. 2.7  10-2 M-2•s-1
c. 1.6  10-4 M-2•s-1
d. 8.1  10-3 M-2•s-1
e. 9.0  10-2 M-2•s-1
____ 38. Rate data have been determined at a particular temperature for the overall reaction
2NO + 2H2
N2 + 2H2O in which all reactants and products are gases. The value of the specific rate
constant at this temperature is ____.
Trial Run
1
2
Initial [NO]
0.10 M
0.10 M
Initial [H2]
0.20 M
0.30 M
Initial Rate (M•s-1)
0.0150
0.0225
3
0.20 M
0.20 M
0.0600
a. 0.75 M-1•s-1
b. 7.5 M-2•s-1
c. 3.0  10-3 M-2•s-1
d. 3.0  10-4 M-1•s-1
e. 375 M-2•s-1
____ 39. Consider a chemical reaction involving compounds A and B, which is found to be first order in A and second
order in B. At what rate will the reaction occur in experiment 2?
Rate (M•s-1)
0.10
?
Experiment
1
2
Initial [A]
1.0 M
2.0 M
Initial [B]
0.20 M
0.60 M
a. 1.2 M•s-1
b. 0.20 M•s-1
c. 0.60 M•s-1
d. 1.8 M•s-1
e. 0.36 M•s-1
____ 40. The oxidation of NO by O3 is first order in each of the reactants, and its rate constant is 1.5  107 M-1•s-1. If
the concentrations of NO and O3 are each 5.0  10-7 M, what is the rate of oxidation of NO in M•s-1?
a. 3.8  10-6
b. 2.5  10-14
c. 7.5  10-7
d. 15
e. 7.5
____ 41. A bimolecular reaction is found to be 1st order with respect to both reactants. If the rate of reaction is 1.87
mol/L •s at 25°C, what is the reaction rate if both reactant concentrations are doubled?
a. 7.48 mol/L •s
b. 46.8 mol/L •s
c. 1.87 mol/L •s
d. 0.94 mol/L •s
e. 3.74 mol/L •s
____ 42. Consider the hypothetical reaction and rate data below. Determine the form of the rate-law expression (i.e.,
determine the values of a and b in rate = k[A]a[B]b) and also the value of the specific rate constant, k. Which
of the answers below would be the initial rate of reaction for [A]initial = 0.40 M and [B]initial = 0.10 M?
3A + 2B Products
Run
1
2
3
a.
b.
c.
d.
e.
[A]initial
0.10 M
0.20 M
0.30 M
1.6  10-4 M•s-1
3.4  10-3 M•s-1
1.2  10-3 M•s-1
4.8  10-4 M•s-1
6.4  10-3 M•s-1
[B]initial
0.10 M
0.30 M
0.10 M
Initial Rate of Reaction
(moles per liter per second)
4.0  10–4
4.8  10–3
3.6  10–3
____ 43. Rate data have been determined at a particular temperature for the overall reaction
2NO + 2H2
+ 2H2O
in which all reactants and products are gases.
Trial Run
1
2
3
____ 44.
____ 45.
____ 46.
____ 47.
____ 48.
Initial [NO]
0.10 M
0.10 M
0.20 M
Initial [H2]
0.20 M
0.30 M
0.20 M
Initial Rate (M•s-1)
0.0150
0.0225
0.0600
What would be the initial rate of the reaction if the initial molar concentration of NO = 0.30 M and the initial
molar concentration of H2 = 0.10 M?
a. 0.068 M•s-1
b. 0.22 M•s-1
c. 0.022 M•s-1
d. 0.040 M•s-1
e. 0.10 M•s-1
The half-life for the reactant A in the first order reaction A
B is 36.2 seconds. What is the rate constant for
this reaction at the same temperature?
a. 52.2 s-1
b. 0.0276 s-1
c. 0.0191 s-1
d. 18.1 s-1
e. 0.00832 s-1
The rate constant for the first order reaction A B + C is k = 3.3  10-2 min-1 at 57 K. What is the half-life
for this reaction at 57 K?
a. 21 min
b. 30 min
c. 61 min
d. 9.1 min
e. 1200 min
The rate constant for the second order reaction 2NO2
N2O4 is 2.79 L/mol •min at 48°C. If the initial
concentration of NO2 is 1.05 M , what is the half-life?
a. 20.5 s
b. 10.3 s
c. 0.341 min
d. 176 s
e. 14.9 s
The half-life of the zero order reaction A B is 0.56 minutes. If the initial concentration of A is 3.4 M, what
is the rate constant?
a. 6.07 mol/L •min
b. 1.24 mol/L •min
c. 3.04 mol/L •min
d. 0.619 mol/L •min
e. 1.79 mol/L •min
The decomposition of dimethylether at 504°C is first order with a half-life of 1570. seconds. What fraction of
an initial amount of dimethylether remains after 4710. seconds?
a. 1/3
b. 1/6
c. 1/8
d. 1/16
____ 49.
____ 50.
____ 51.
____ 52.
e. 1/32
The decomposition of dinitrogen pentoxide obeys the rate-law expression rate = 0.080 min-1[N2O5]. If the
initial concentration of N2O5 is 0.30 M, what is the concentration after 2.6 minutes?
N2O5
N2O3 + O2
a. 0.38 M
b. 0.028 M
c. 0.24 M
d. 0.13 M
e. 0.32 M
A molecule of ethyl alcohol is converted to acetaldehyde in one's body by zero order kinetics. If the
concentration of alcohol is 0.015 mol/L and the rate constant = 6.4  10-5 mol/L•min, what is the
concentration of alcohol after 3.5 hours?
a. 0.0016 mol/L
b. 9.6  107 mol/L
c. 4.3  10-3 mol/L
d. 0.15 mol/L
e. 0.0032 mol/L
A chemical reaction A B + C is first order in A and has a rate constant of 1.2  10-3 min-1. If the initial
concentration of A is 0.40 M., how much time must pass in order to reduce the concentration of A to 0.22 M?
a. 5.0  102 min
b. 3.0  102 min
c. 7.4  10-3 min
d. 4.3  10-4 min
e. 2.2  102 min
The gas phase reaction below obeys the rate-law expression rate = k[SO2Cl2]. At 593 K the specific rate
constant is 2.2  10-5 s-1. A 2.0-g sample of SO2Cl2 is introduced into a closed 4.0-L container.
SO2Cl2
SO2 + Cl2
How much time must pass in order to reduce the amount of SO2Cl2 present to 1.8 grams?
a. 7.4  103 seconds
b. 2.1  102 seconds
c. 3.5  102 seconds
d. 4.8  103 seconds
e. 5.8  104 seconds
____ 53. The gas phase reaction below obeys the rate-law expression rate = k[PCl5]. At 400 K
the specific rate constant is 0.0371 min-1. How many hours are required to reduce a sample of PCl5 to 10% of
its original amount?
PCl5 PCl3 + Cl2
a. 3.10 hrs
b. 1.03 hrs
c. 186 hrs
d. 3.71 hrs
e. 62 hrs
____ 54. Consider the following first order reaction.
A2B AB + A
If it takes 87 seconds for the concentration of A2B to be reduced from 2.2 M to 0.12 M, what is the value of
the specific rate constant?
a. 0.0334 min-1
b. 2.01 min-1
c. 2.01 s-1
d. 18.3 min-1
e. 3.51  10-3 s-1
____ 55. The reaction SF4 SF2 + F2 has the following rate law:
rate = 0.011 L/mol•s [SF4]2.
How many minutes will it take for the concentration of SF4 to be reduced from 2.5 M to 0.25 M?
a. 327 min
b. 0.025 min
c. 5.5 min
d. 0.040 min
e. 22.7 min
____ 56. Cyclopropane rearranges to form propene in a reaction that is first order. If the rate constant is 2.74  10-3 s-1,
how long would it take for 85.6% of the cyclopropane to rearrange if the initial concentration was 0.460 M?
a. 51.0 s
b. 62.0 s
c. 707 s
d. 2.74  10-3 s
e. 3.83  10-4 s
____ 57. At 300 K the reaction below obeys the rate law Rate =k[NOCl]2 where k = 2.8  10-5 M-1•s-1.
2NOCl 2NO + Cl2
Suppose 1.0 mole of NOCl is introduced into a 2.0-liter container at 300 K. Evaluate the half-life of the
reaction.
a. 2.6  103 seconds
b. 3.6  104 seconds
c. 2.4  104 seconds
d. 1.1  103 seconds
e. 4.0  104 seconds
____ 58. The second order reaction
2CH4
C2H2 + 3H2
has a rate constant of 5.76 M-1•min-1 at 1600 K. How long would it take for the concentration of CH4 to be
reduced from 0.89 M to 5.25  10-4 M?
a. 165 hrs
b. 0.15 hrs
c. 2.75 hrs
d. 5.51 hrs
e. 9.27 hrs
____ 59. Compounds A and B react to form C and D in a reaction that is found to be second-order overall and secondorder in B. The rate constant at 50.°C is 2.48 liter per mole per minute. What is the half-life of B (in min) if
0.822 M B reacts with excess A?
A+B C+D
a. 0.0139
b. 12.0
c. 1.39
d. 0.491
e. 5.88
____ 60. At 100 K the reaction below obeys the rate law rate = k[AB2]2 where k = 5.7 M-1•s-1.
2AB2
A2 + 2B2
What would the concentration of AB2 be after 60 minutes if the initial concentration was 1.45 mol/L?
a. 4.9  10-5 M
b. 2.0  10-5 M
c. 1.2  10-2 M
d. 2.4  10-5 M
e. 1.9  10-4 M
____ 61. At a certain temperature the reaction 2B C + D obeys the rate-law expression rate = (1.14  10-3 M-1•s1
)[B]2. If 5.00 mol of B is initially present in a 1.00-L container at that temperature, how long would it take
for 2.00 mol of B to be consumed at constant temperature?
a. 224 s
b. 87.5 s
c. 46.0 s
d. 73.0 s
e. 58.5 s
____ 62. Compounds A and B react to form C and D in a reaction that is found to be second-order overall and secondorder in B. The rate constant at 30°C is 0.622 liter per mole per minute.
A+B C+D
How many minutes does it take 4.0  10-2 M B (mixed with excess A) to be reduced to 3.3  10-2 M B?
a. 1.4 min
b. 3.6 min
c. 5.0 min
d. 6.4 min
e. 8.5 min
____ 63. A plot of
versus time is linear for the reaction D
E. What is the kinetic order of the reaction?
a. second
b. first
c. zero
d. one-half
e. negative one
____ 64. A plot of ln [C] versus time is linear for the reaction C
D. What is the kinetic order of the reaction?
a. second
b. first
c. zero
d. one-half
e. negative one
____ 65. Which statement is incorrect?
a. The reaction rate for a zero-order reaction is independent of concentrations.
b. The specific rate constant for a second-order reaction is independent of temperature.
c. The half-life for a first-order reaction is independent of initial concentrations.
d. The rate law expression relates rate and concentration.
e. The integrated rate equation relates time and concentration.
____ 66. Which of the following statements concerning graphical methods for determining reaction order is false?
a. For a first-order reaction the plot of ln [A] vs. time gives a straight line.
b. For a first-order reaction the slope of the straight-line graph equals -ak.
____ 67.
____ 68.
____ 69.
____ 70.
____ 71.
____ 72.
c. For a second-order reaction the plot of [A]2 vs. time gives a straight line.
d. For a first-order reaction the intercept of the straight-line graph equals ln [A]0.
e. For a zero-order reaction the plot of [A] vs. time gives a straight line.
Which idea listed below is not a part of the collision theory of reaction rates?
a. Molecules must be properly oriented when they collide to react.
b. Molecules must collide to react.
c. Molecules must collide with enough kinetic energy to overcome the potential energy
stabilization of the bonds.
d. Effective collisions result in a chemical reaction.
e. All molecular collisions result in a reaction.
Which one of the following statements is false?
a. In order for a reaction to occur, reactant molecules must collide with each other.
b. A catalyst alters the rate of a reaction and is neither a product nor a reactant in the overall
equation.
c. According to collision theory a three-body collision is less likely than a two-body
collision.
d. In reactions that are second order in one reactant and first order in another, the slow step
generally involves a three-body collision of these reactants.
e. The transition state is a short-lived, high energy state, intermediate between reactants and
products.
Which of the following statements regarding collision and transition state theory is false?
a. Reactants must collide to form products.
b. All reactant collisions result in product formation.
c. Activation energy is always positive.
d. Reactant molecules must absorb energy to form the transition state.
e. Reactant collisions must be oriented properly to form products.
Which statement is false?
a. If a reaction is thermodynamically spontaneous, it may occur rapidly.
b. A fast reaction may be thermodynamically spontaneous.
c. If a reaction is thermodynamically spontaneous, it may occur slowly.
d. If a reaction is thermodynamically spontaneous, it must have a low activation energy.
e. Rate of reaction is a kinetic quantity rather than a thermodynamic quantity.
Which term is incorrectly matched with its description?
a. Activation Energy/ kinetic energy required for reaction to occur
b. Transition State/ short-lived high-energy intermediate state
c. Effective Collision/ molecular collision resulting in a reaction
d. Net energy change of the reaction/ Ea,forward - Ea, reverse
e. Exothermic Reaction/ reaction having Ea, reverse > Ea,forward
A reaction has an activation energy of 40 kJ and an overall energy change of reaction of -100 kJ. In each of
the following potential energy diagrams, the horizontal axis is the reaction coordinate and the vertical axis is
potential energy in kJ. Which potential energy diagram best describes this reaction?
a.
c.
e.
b.
d.
____ 73. Given the following potential energy diagram for the one-step reaction
X+Y Z+R
The reaction ____.
a. releases energy
b. absorbs energy
c. is impossible
d. occurs without a net change in energy
e. may either absorb or release energy
____ 74. Given the following potential energy diagram for the one-step reaction
X+Y Z+R
The arrow "d" represents the ____.
a. energy content of products
b. activation energy for the forward reaction
c. energy content of reactants
d. activation energy for the reverse reaction
e. the net change in energy for the reaction
____ 75. Given the following potential energy diagram for the one-step reaction
X+Y Z+R
The activation energy of the reverse reaction is equal to ____.
a. d
b. c plus d
c. c
d. a plus c
e. d minus a
____ 76. Given the following potential energy diagram for the one-step reaction
X+Y Z+R
The arrow "a" represents the ____.
a. energy content of products
b. activation energy for the forward reaction
c. energy content of reactants
d. activation energy for the reverse reaction
e. the net change in energy for the reaction
____ 77. Given the following potential energy diagram for the one-step reaction
X+Y Z+R
The point "b" represents ____.
a. the energy of the mixture when half of the reactants have been converted to products
b. the energy of the transition state
c. the number of moles of transition state that must be formed
d. the energy of the forward reaction
e. the energy of the reverse reaction
____ 78. Given the following potential energy diagram for the one-step reaction
X+Y
____ 79.
____ 80.
____ 81.
____ 82.
Z+R
The arrow "c" represents the ____.
a. net energy of reaction for the forward reaction
b. activation energy for the forward reaction
c. net energy of reaction for the reverse reaction
d. activation energy for the reverse reaction
e. energy content for the reaction
Which of the following statements about reaction mechanisms is false?
a. A reaction can have more than one possible mechanism.
b. A reaction mechanism must be consistent with the experimentally observed rate law.
c. The slowest step in the reaction mechanism is called the rate-determining step.
d. Reaction mechanisms involve complex reaction steps.
e. Reaction mechanisms are difficult to prove.
A reaction mechanism will usually be
a. the only possible explanation for the reaction.
b. difficult to verify experimentally.
c. proven experimentally to be the balanced chemical equation.
d. obvious from a consideration of the balanced chemical equation.
e. obvious from a consideration of the reaction rate data.
Which of the following is a kinetics concept?
a. free energy
b. enthalpy
c. spontaneity
d. reaction mechanism
e. entropy
Consider the hypothetical reaction shown below.
A + 2B AB2
Assume that the following proposed mechanism is consistent with the rate data.
B
B2
B
A
+
+
+
+
B B2
A AB + B
AB AB2
2B AB2
slow
fast
fast
overall
Which one of the following statements must be true? The reaction is ____.
a. first order in A, second order in B, and third order overall
b. second order in B and second order overall
c. first order in A and first order overall
d. second order in B, zero order in A, and third order overall
e. second order in A and second order overall
____ 83. Consider the hypothetical reaction shown below.
2A + C2 A2C + C
Assume that the following proposed mechanism is consistent with the rate data.
A
AC
2A
+
+
+
C2
A
C2
AC + C
A2C
A2C + C
slow
fast
overall
Which one of the following statements must be true? The reaction is ____.
a. first order in A, first order in B, and third order overall
b. second order in C2 and second order overall
c. first order in A and first order in C2
d. second order in C2, zero order in A, and third order overall
e. second order in A and second order overall
____ 84. Consider the following proposed mechanism. If this mechanism for the overall reaction were correct, and if k1
were much less than k2, then the observed rate law would be
2A
I+B
C+I
C+D
a. rate =k1[A]
b. rate =k2[I][B]
c. rate =k1[A]2
d. rate =k1[A]2 -k2[C][D]
e. rate =k1k2[A]2[I][B]
____ 85. Suppose the reaction
2AB + C2
A2C + B2C
occurs by the following mechanism.
Step 1
Step 2
Step 3
Step 4
Overall
AB
B
AC2
A2C2
+
+
+
+
2 AB
C2 AC2
AB AB2
AB2
A2C2
B2 A2C
+ C2
+
+
+
A2C
B
B2
B2C
+ B2C
slow
fast
fast
fast
The rate law expression must be rate = ____.
a. k[AB][C2]
b. k[AB]2[C2]
c. k[AB]2
d. k[AB]
e. k[C2]
____ 86. Assume the following reaction
3H2 + CO CH4 + H2O
occurs by the given reaction mechanism.
Step 1
H2
+ CO
H2CO
slow
Step 2
Step 3
Overall
H2
H2
+ H2CO
CH4 + O
+ O H2O
3H2 + CO
CH4 + H 2O
fast
fast
The rate law expression must be rate = ____.
a. k[H2]2[CO]2
b. k[H2]2[CO]
c. k[H2][CO]2
d. k[H2][CO]
e. k[H2]2[CO]3
____ 87. Consider the reaction below and its observed rate law expression. Which proposed mechanisms are
consistent with the rate law expression?
2NO2
2NO + O2
rate =k[NO2]2
I.
NO2 + NO2
N2O4
N2O4
N2 + 2O2
N2 + O2
2NO
2NO2
2NO + O2
slow
fast
fast
overall
II.
NO2
N + O2
NO2 + N N2O2
N2O2
2NO
2NO2
2NO + O2
slow
fast
fast
overall
III.
NO2
NO + O
O + NO2
NO + O2
2NO2
2NO + O2
slow
fast
overall
a. I
b. II
c. III
d. I and III
e. another combination
____ 88. Which statement concerning a possible mechanism for a reaction is false?
a. A possible mechanism must be consistent with the experimental data.
b. Each elementary step is represented by a balanced equation.
c. The elementary steps must add to give the equation for the overall reaction.
d. The speed of the slow step limits the rate at which the overall reaction occurs.
e. For all reactions the experimentally determined reaction orders of the reactants indicate
the number of molecules of those reactants involved in the slow step of the mechanism.
____ 89. Which of the following statements concerning a reaction and its mechanism is false?
a. For a reactant, more is consumed than is formed.
b. For a product, more is formed than is consumed.
c. A reaction intermediate is formed in early steps and completely consumed in later steps.
d. For a multi-step mechanism, the slowest step has the highest activation energy.
e. Reactions involving simultaneous trimolecular collisions are very common in gases.
____ 90. Reaction rates increase with increasing temperature because ____.
a. the activation energy increases
b. larger molecules collide more frequently
c. the energy of the transition state is lowered
d. the activation energy is decreased
e. a greater fraction of molecules possess the activation energy when they collide
____ 91. Which of the following statements regarding temperature and reaction rate is false.
a. The Arrhenius equation can be used to find the activation energy of a reaction.
b. Reaction rate always increases with higher temperature.
c. A larger negative value of G0 causes a faster reaction rate.
d. A larger value of Ea causes a slower reaction rate.
e. The rate constant for a reaction decreases at lower temperatures.
____ 92. Suppose the activation energy of a certain reaction is 250 kJ/mol. If the rate constant at T1 = 300 K is k1, and
the rate constant at T2 = 320 K is k2, then k2/k1 = ____. (The universal gas constant = 8.314 J/mol•K.)
a. 3  10-29
b. 0.067
c. 15.0
d. 525
e. 3  1028
____ 93. Suppose the activation energy of a certain reaction is 250 kJ/mol. If the rate constant at T1 = 300 K is k1, and
the rate constant at T2 = 320 K is k2, then k2/k1 = ____. (The universal gas constant = 8.314 J/mol•K.)
a. 3  10-29
b. 0.067
c. 15.0
d. 525
e. 3  1028
____ 94. The specific rate constant, k, for a reaction is 2.64  10-2 s-1 at 25°C, and the activation energy is 74.0 kJ/mol.
Calculate k at 50°C. (The universal gas constant = 8.314 J/mol•K.)
a. 0.832 s-1
b. 71.9 s-1
c. 0.266 s-1
d. 1.08 s-1
e. 0.0265 s-1
____ 95. The specific rate constant, k, for a reaction is 0.44 s-1 at 298 K, and the activation energy is 245.kJ/mol.
Calculate k at 398 K. (The universal gas constant = 8.314 J/mol•K.)
a.
b.
c.
d.
e.
2.71  1010 s-1
6.17  1010 s-1
1.03  1010 s-1
8.32  108 s-1
4.51  109 s-1
____ 96. The rate constant for a first-order reaction is 0.58 s-1 at 25°C. At what temperature would the rate constant
have a value of 0.75 s-1? The activation energy is 84 kJ/mol and the universal gas constant = 8.314 J/mol•K.
____ 97.
____ 98.
____ 99.
____ 100.
a. 30°C
b. 300°C
c. 298 K
d. 301 K
e. 310 K
The specific rate constant, k, for a reaction is 2.64  10-2 s-1 at 25°C, and the activation energy is 74.0 kJ/mol.
Calculate k at 50°C.
a. 0.832 s-1
b. 71.9 s-1
c. 0.266 s-1
d. 1.08 s-1
e. 0.0265 s-1
The rate constant, k, for a first-order reaction is 1.20  102 s-1 at 45°C and the activation energy is 98.2 kJ/mol.
Calculate the rate constant for this reaction at 95°C.
a. 1.87  104 s-1
b. 7.72  10-1 s-1
c. 6.06  10-2 s-1
d. 1.40  103 s-1
e. 2.02  105 s-1
The rate constant, k, for a first-order reaction is 1.36  103 s-1 at 90.°C and the activation energy is 78.4
kJ/mol. Calculate the rate constant for this reaction at 50.°C.
a. 60.4 s-1
b. 54.5 s-1
c. 23.8 s-1
d. 4.85 s-1
e. 1.78  103 s-1
Calculate the activation energy of a reaction if the rate constant is 0.75 s-1 at 25°C and 11.5 s-1 at 75°C. (The
universal gas constant = 8.314 J/mol•K.)
a. 681 J/mol
b. 20.4 kJ/mol
c. 15.8 kJ/mol
d. 47.1 kJ/mol
e. 31.4 kJ/mol
____ 101. Calculate the activation energy of a reaction if the rate constant is 0.75 s-1 at 25°C and 11.5 s-1 at 75°C.
a. 681 J/mol
b. 20.4 kJ/mol
c. 15.8 kJ/mol
d. 47.1 kJ/mol
e. 31.4 kJ/mol
____ 102. Calculate the activation energy of a reaction if its rate constant is 2.8  106 s-1 at 24°C and 1.5  107 s-1 at
48°C.
a. 26 kJ/mol
b. 80. kJ/mol
c. 55 kJ/mol
d. 67 J/mol
e. 3.51 J/mol
____ 103. What would be the activation energy of a reaction if its rate constant at 35°C was double the value of its rate
constant at 25°C?
a. 63.8 kJ/mol
b. 75.1 kJ/mol
c. 8.12 kJ/mol
d. 52.9 kJ/mol
e. 68.3 J/mol
____ 104. A catalyst ____.
a. is used up in a chemical reaction
b. changes the value of G0 of the reaction
c. is always a solid
d. does not influence the reaction in any way
e. changes the activation energy of the reaction
____ 105. A catalyst
a. increases the amount of products present at equilibrium.
b. increases the rate at which equilibrium is reached but decreases the equilibrium constant.
c. increases the rate at which equilibrium is reached without changing the equilibrium
constant.
d. increases H for the process.
e. lowers S for the process.
____ 106. Which of the following statements about catalysts are false?
a. A catalyst lowers the activation energy.
b. A catalyst can make a nonspontaneous reaction spontaneous.
c. A catalyst speeds up both the forward and reverse reaction.
d. A catalyst speeds up the rate of reaction.
e. Catalyst are often transition metals and transition metal oxides.
____ 107. Which of the following is not an example of an important, useful reaction catalyzed by transition metals
and/or their oxides?
a. the Haber process for the production of ammonia
b. the contact process for the production of sulfur trioxide in producing sulfuric acid
c. the hydrogenation of unsaturated hydrocarbons
d. the reaction of leaded fuels with the catalysts in catalytic converters
e. the chlorination of benzene
____ 108. The catalytic converters installed in newer models of automobiles are designed to catalyze certain kinds of
favorable reactions. Unfortunately, other unfavorable reactions also are catalyzed. Which one of those listed
below, all of which are catalyzed in such mufflers, is an unfavorable reaction?
a. 2CO(g) + O2(g)
2CO2(g)
b. 2C8H18(g) + 25O2(g)
16CO2(g) + 18H2O(g)
c. C(s) + O2(g)
CO2(g)
d. 2SO2(g) + O2(g)
2SO3(g)
e. 2NO(g)
N2(g) + O2(g)
____ 109. Which statement concerning biological catalysts is false?
a.
b.
c.
d.
e.
Enzymes are proteins that act as catalysts for specific biochemical reactions.
The reactants in enzyme-catalyzed reactions are called substrates.
Each enzyme catalyzes many different reactions in a living system.
Enzyme-catalyzed reactions are important examples of zero-order reactions.
Discovery or synthesis of catalysts that mimic the efficiency of naturally occurring
enzymes would saved on the costs of using high temperature and high pressure in
commercial processes.
____ 110. The reaction, A + 2B B2 + A, proceeds by the following mechanism: (A is a catalyst.)
A + B AB
AB + B B2 + A
(slow)
(fast)
What is the rate law expression for this reaction?
a. Rate =k[A]
b. Rate =k[B]
c. Rate =k[A][B]
d. Rate =k[A][B]2
e. Rate =k[A]2[B]
____ 111. Consider the following hypothetical reaction: A + B  C.
Pure A, B and C are mixed together, all at the same concentration, 0.250 M. After 5.00 minutes, the
concentration of C is found to be 0.474 M. Calculate the average rate of the reaction.
a. 0.0948 M·min-1
b. 0.224 M·min-1
c. 0.0448 M·min-1
d. 22.3 M·min-1
____ 112. The rate expression for the following reaction is found to be: Rate = k[N2O5]
2N2O5(g)  4NO2(g) + O2(g)
What is the overall order of the reaction?
a. first order
b. second order
c. third order
d. fourth order
____ 113. For the reaction 2A + B  C, the rate-law expression is
a. rate = k [ A ]2 [ B ].
b. rate = k [ A ]2.
c. rate = k [ A ] [ B ].
d. determined only from experimental data.
____ 114. Cyclopropane rearranges to form propene in a reaction that is first order. If the rate constant is 2.74  10-3
s-1, how long would it take for the concentration of the cyclopropane to be reduced to 0.0662 M if the initial
concentration was 0.460 M?
a. 144 s
b. 2.54  103 s
c. 707 s
d. 1.41  10-3 s
____ 115. The decomposition of dimethyl ether at 504°C is first order with a half-life of 1570 s. What fraction of an
initial amount of dimethyl ether remains after 4710 seconds?
a. 1/3
b. 1/6
c. 1/8
d. 1/16
____ 116. According to the collision theory of reaction rates, for a reaction to occur, molecules, atoms, or ions must first
collide. The rate of a reaction can be expressed as the product of three factors. Which one of the following is
NOT one of these factors?
a. total number of collisions per cubic centimeter per second
b. fraction of collisions with intermolecular forces
c. fraction of collisions with sufficient energy
d. fraction of collisions with proper orientation
____ 117. Many organic compounds containing bromide can undergo a type of reaction called nucleophilic substitution,
in which the bromide is replaced by another atom or group of atoms, such as hydroxide: R-Br + OH-  R-OH
+ Br-, where R represents a group of carbon and hydrogen atoms. There are two possible reaction
mechanisms, depending, in part, on the structure of the R group.
(a)
Substitution Nucleophilic Unimolecular, or SN1, has two steps:
(1)
(2)
(b)
R-Br  R+ + BrR+ + OH- R-OH
(slow)
(fast)
Substitution Nucleophilic Bimolecular, or SN2, has one step, with a notable transition state:
(1)
OH- + R-Br  HO R Br  HO-R + Br- (HO-R is the same as R-OH)
The nucleophilic substitutions of 2-bromo-2-methylpropane, (CH3)3C-Br, and bromomethane,
CH3-Br, have been studied and experimentally found to follow the rate law expressions:
(CH3)3C-Br + OH- (CH3)3C-OH + BrCH3-Br + OH- CH3-OH + Br-
rate = k[(CH3)3C-Br]
rate = k[CH3-Br][OH-]
Which reaction mechanism is consistent with the given kinetic data for the nucleophilic substitution of each
compound?
a. (CH3)3C-Br: SN1 and CH3-Br: SN1
b. (CH3)3C-Br: SN1 and CH3-Br: SN2
c. (CH3)3C-Br: SN2 and CH3-Br: SN1
d. (CH3)3C-Br: SN2 and CH3-Br: SN2
____ 118. According to L. Kunigk, et al. [Braz. J. Chem. Eng., 18, 217 (2001)], peracetic acid, CH3COOOH, (also
called peroxyacetic acid) is a powerful sanitizer, but it has a high rate of decomposition. The activation energy
for the decomposition is 66.20 kJ/mol and the rate constant at 25°C is 1.71  10-3 h-1.
At what temperature would the rate constant be 9.64  10-3 h-1?
a. 46°C
b. 105°C
c. 32°C
d. 1407°C
____ 119. Methyl butyrate,
, is an ester that has the smell of apples. In the presence of
strong acids, it rapidly hydrolyses (splits by reaction with water). A proposed mechanism has these steps:
(1)
(2)
(3)
(4)
(5)
Overall:
What is the catalyst in this reaction?
a. H2O
b.
c.
d. H+
____ 120. Although more than 95% of all catalysts industrially are heterogeneous, there are certainly some important
chemicals produced using a homogeneous catalyst. Of the industrial processes identified below by their
chemical equations, most are homogeneous.
Which one is heterogeneous?
a. The oxidation of sulfur dioxide, SO2, to sulfur trioxide, SO3, in the manufacture of sulfuric
acid (the contact process):
b. The hydroformylation of alkenes (the oxo process):
c. The oxidation of alkenes (the Wacker-Hoechst process):
d. The carbonylation of methanol to acetic acid (the Monsanto process):
Kinetics
Answer Section
MULTIPLE CHOICE
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TOP:
39. ANS:
40. ANS:
D
PTS: 1
TOP: The Rate of a Reaction
C
PTS: 1
TOP: The Rate of a Reaction
A
PTS: 1
TOP: The Rate of a Reaction
E
PTS: 1
TOP: The Rate of a Reaction
B
PTS: 1
TOP: The Rate of a Reaction
A
PTS: 1
TOP: The Rate of a Reaction
D
PTS: 1
TOP: Nature of the Reactants
E
PTS: 1
TOP: Nature of the Reactants
C
PTS: 1
TOP: Nature of the Reactants
C
PTS: 1
TOP: Nature of the Reactants
E
PTS: 1
TOP: Nature of the Reactants
C
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
D
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
C
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
C
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
A
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
B
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
E
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
A
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
E
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
B
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
D
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
A
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
E
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
A
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
B
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
C
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
D
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
C
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
B
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
D
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
E
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
E
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
D
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
C
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
C
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
E
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
B
PTS: 1
DIF: * Harder Question
Concentrations of Reactants: the Rate-Law Expression
D
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
A
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
41. ANS: A
PTS: 1
TOP: Concentrations of Reactants: the Rate-Law Expression
42. ANS: E
PTS: 1
DIF: * Harder Question
TOP: Concentrations of Reactants: the Rate-Law Expression
43. ANS: A
PTS: 1
DIF: * Harder Question
TOP: Concentrations of Reactants: the Rate-Law Expression
44. ANS: C
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
45. ANS: A
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
46. ANS: B
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
47. ANS: C
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
48. ANS: C
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
49. ANS: C
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
50. ANS: A
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
51. ANS: A
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
52. ANS: D
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
53. ANS: A
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
54. ANS: B
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
55. ANS: C
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
56. ANS: C
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
57. ANS: B
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
58. ANS: C
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
59. ANS: D
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
60. ANS: D
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
61. ANS: E
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
62. ANS: E
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
63. ANS: A
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
64. ANS: B
PTS: 1
TOP: Concentration Versus Time: The Integrated Rate Equation
65. ANS: B
PTS: 1
TOP:
66. ANS:
TOP:
67. ANS:
68. ANS:
69. ANS:
70. ANS:
71. ANS:
72. ANS:
73. ANS:
74. ANS:
75. ANS:
76. ANS:
77. ANS:
78. ANS:
79. ANS:
80. ANS:
81. ANS:
82. ANS:
83. ANS:
84. ANS:
TOP:
85. ANS:
86. ANS:
87. ANS:
88. ANS:
89. ANS:
90. ANS:
91. ANS:
92. ANS:
93. ANS:
94. ANS:
95. ANS:
96. ANS:
97. ANS:
98. ANS:
99. ANS:
100. ANS:
101. ANS:
102. ANS:
103. ANS:
104. ANS:
105. ANS:
106. ANS:
107. ANS:
108. ANS:
109. ANS:
Concentration Versus Time: The Integrated Rate Equation
C
PTS: 1
DIF: * Harder Question
Concentration Versus Time: The Integrated Rate Equation
E
PTS: 1
TOP: Collision Theory of Reaction Rates
D
PTS: 1
TOP: Transition State Theory
B
PTS: 1
TOP: Transition State Theory
D
PTS: 1
TOP: Transition State Theory
E
PTS: 1
TOP: Transition State Theory
A
PTS: 1
TOP: Transition State Theory
A
PTS: 1
TOP: Transition State Theory
E
PTS: 1
TOP: Transition State Theory
B
PTS: 1
TOP: Transition State Theory
B
PTS: 1
TOP: Transition State Theory
B
PTS: 1
TOP: Transition State Theory
D
PTS: 1
TOP: Transition State Theory
D
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
B
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
D
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
B
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
C
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
C
PTS: 1
DIF: * Harder Question
Reaction Mechanisms and the Rate-Law Expression
A
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
D
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
A
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
E
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
E
PTS: 1
TOP: Reaction Mechanisms and the Rate-Law Expression
E
PTS: 1
TOP: Temperature: The Arrhenius Equation
C
PTS: 1
TOP: Temperature: The Arrhenius Equation
D
PTS: 1
TOP: Temperature: The Arrhenius Equation
D
PTS: 1
TOP: Temperature: The Arrhenius Equation
C
PTS: 1
TOP: Temperature: The Arrhenius Equation
A
PTS: 1
TOP: Temperature: The Arrhenius Equation
B
PTS: 1
TOP: Temperature: The Arrhenius Equation
C
PTS: 1
TOP: Temperature: The Arrhenius Equation
A
PTS: 1
TOP: Temperature: The Arrhenius Equation
B
PTS: 1
TOP: Temperature: The Arrhenius Equation
D
PTS: 1
TOP: Temperature: The Arrhenius Equation
D
PTS: 1
TOP: Temperature: The Arrhenius Equation
C
PTS: 1
TOP: Temperature: The Arrhenius Equation
D
PTS: 1
TOP: Temperature: The Arrhenius Equation
E
PTS: 1
TOP: Catalysts
C
PTS: 1
TOP: Catalysts
B
PTS: 1
TOP: Catalysts
D
PTS: 1
TOP: Catalysts
D
PTS: 1
TOP: Catalysts
C
PTS: 1
TOP: Catalysts
110.
111.
112.
113.
114.
115.
116.
117.
118.
119.
120.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
C
C
A
D
C
C
B
B
A
D
A
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
1
TOP:
TOP:
TOP:
TOP:
TOP:
Catalysts
Additional Questions
Additional Questions
Additional Questions
Additional Questions
TOP:
TOP:
TOP:
TOP:
TOP:
Additional Questions
Additional Questions
Additional Questions
Additional Questions
Additional Questions